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![D. 13.0
37. Compute the concentration of hydroxide ion, [OH-] in 0.2 M HF. Given
Ka for HF is 6.6 x 10. *
O A. 1.32 x 10-4 M
O B. 1.74 x 10-6 M
O C. 5.74 x 10-9 M
O D. 8.70 x 10-13 M
0.42 M for formic acid, HCOOH solution. The va](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4e08145-6633-48c3-b58e-2d1048230a96%2F29f3afd2-96b6-4438-9de4-bed9ca78416c%2Fcvi7ne_processed.jpeg&w=3840&q=75)
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- A.) The value of Ka for hydrocyanic acid is 4.00×10-10.What is the value of Kb, for its conjugate base, CN-? B.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of benzoic acid, C6H5COOH to be 2.199.Use the information she obtained to determine the Ka for this acid.Ka(experiment) =Write the equations that represent the first and third ionization steps for phosphoric acid (H3PO4) in water. (Use H3O+ instead of H+.) first ionization step: + H2O(l) + third ionization step: + H2O(l) + --- The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-? --- The value of Ka for nitrous acid is 4.50×10-4.What is the value of Kb, for its conjugate base, NO2-?Calculate the volume (ml)of concentrated ammonia and the weight (gm) of ammonium chloride respectively to be taken to prepare 100 ml of buffer solution at a pH of 10 if the final concentration of the salt is 0.20 mol. Note that the molar concentration of concentrated ammonia is equal to 14.8 mol/liter, and that the pKb of ammonia is 4.76, and the molecular weight of ammonium :chloride 53.5 g/mole.lt is about
- The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.21. calculate the H+ in M for 0.620 M C2H5NH3Cl solution. Kb for solution is 5.60•10^-4A 0.10 M solution of formic acid (HCOOH) is prepared in various solvents: a. Pure water b. 0.10 M NaHCOO solution c. 0.10 M Ca(HCOO)2 solution d. 0.10 M of NaCl Compute the pH of each solution. The Ka of formic acid os 1.78×10-4. Show also the ICE table and all partinent solutions
- Considering the equilibrium below, which of the following is/are TRUE? CH3OH + HNO2 = CH3OH2+ + NO2- CH3OH is a base NO2 is a conjugate acid IAM. I only SXY. II only AND. I and II IKI. Neither I nor II Which of the following statements is/are ALWAYS TRUE? A higher Ksp value equates to a higher solubility regardless of the salt type When Qsp = Ksp, the system is at equilibrium CHM. I only EQU. II only LIB. I and II RIA. Neither I nor IIHow to answer for Ka/ Kb and calculated pH of a solution?I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Given: In a 10.0 mL 0.10 M CH3COOH solution, a 15 mL 1.00 M HCl solution was added. Compute for it's ka/kb and pH.a) Enough of a monoprotic acid is dissolved in water to produce a 1.291.29 M solution. The pH of the resulting solution is 2.832.83. Calculate the Ka for the acid. b) i) Determine the [OH−] , pH, and pOH of a solution with a [H+] of 8.6×10−10 M at 25 °C. ii) Determine the [H+] , pH, and pOH of a solution with an [OH−] of 0.028 M at 25 °C. iii) Determine the[H+] , [OH−] , and pOH of a solution with a pH of 10.26 at 25 °C. iv) Determine the [H+] , [OH−] , and pH of a solution with a pOH of 3.28 at 25 °C.
- The experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is the solution acidic, basic, or neutral? B. Write the balanced net ionic equilibrium reaction. Identify the acid, base, conjugate acid, and conjugate base. Write the cquilibrium expression Kb for the reaction. C. Look up the theoretical pKafrom the CRC Handbook. Please give me all questions solution fast(2). For the buffer system, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer? Given: • 20.0 ml of 3.00 M sodium bicarbonate = conjugate base in molarity [? −] • 50.0 ML OF 2.00 M carbonic acid = weak acid in molarity [??] • 4.30 × 10−7 ?? of carbonic = ??? (acid-dissociation constant) • Base: (a) 15.0 ml of 0.500 M HCl (b) 15.0 ml of 0.750 M NaOHFor H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by systematic method